At the Nangal fertiliser plant in Punjab, hydrogen is produced by the electrolysis of water. This hydrogen is used for the production of ammonia and nitric acid (by oxidation of ammonia). If the average production of ammonium nitrate is $5000 \mathrm{kg}/\mathrm{day}$, the daily consumption of electricity per day is $\mathrm{x} \times {10}^5$. 

Give thevalue of $\mathrm{x}$ to the nearest integer value.

A constant current flowed for $2 \mathrm{h}$ through a potassium iodide solution oxidising the iodide ion to iodine $\left(2{\mathrm{I}}^{-}\to {\mathrm{I}}_2+2{\mathrm{e}}^{-}\right)$.

At the end of the experiment, the iodine was titrated with $21.75 \mathrm{mL}$ of $0.0831 \mathrm{M}$ sodium thiosulphate solution $\left({\mathrm{I}}_2+2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}\to 2{\mathrm{I}}^{-}+{\mathrm{S}}_4{\mathrm{O}}_6^{2-}\right)$.

What was the average rate of current flow in amperes?

Give the answer up to two places of decimal.

A current passes through two cells containing respectively-($\mathrm{i}$) ${\mathrm{CuSO}}_4$ solution between $\mathrm{Cu}$electrode and ($\mathrm{ii}$) ${\mathrm{AgNO}}_3$ solution between $\mathrm{Pt}$electrodes. Calculate the loss or gain in weight of the different electrodes in the time in which $40 \mathrm{cc}$ of oxygen at $\mathrm{NTP}$collects in the second cell. 

First cell $\left\{\begin{array}{l}0.228 \mathrm{g} \mathrm{Cu}\text{ deposited at cathode. }\\ 0.228 \mathrm{g} \mathrm{Cu}\text{ dissolved out from anode }\end{array}\right.$

$\mathrm{Ag}$is electro deposited on a metallic vessel of surface area $800 {\mathrm{cm}}^2$ by passing a current of $0.2$ amp for three hours. Calculate the thickness of silver deposited. (given density is $10.47 \mathrm{g}/\mathrm{cc}$). If thickness $= \mathrm{A}\times {10}^{-4} \mathrm{cm}.$

Give the value of A up to two places of decimal.